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3 October, 23:53

Using enthalpies of formation, calculate the quantity of heat produced when 14.0 g of propane is completely combusted in air under standard conditions. Assume that liquid water is forming

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  1. 4 October, 02:20
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    The balanced chemical reaction here is:

    C3H8 (g) + 5O2 (g) - - > 3CO2 (g) + 4H2O (l)

    Calculating for the molar change in enthalpy:

    Enthalpy change = 3 (-393.5) + 4 (-285.83) - (-103.85) = - 2220.0 kJ/mole

    Now, propane has a molar mass of 44g/mol. So, for us to calculate the heat released by burning 14 grams of propane, we have:

    -2220 kJ/mole * (14g / 44g/mol) = - 706.36 kJ

    Answer:

    -706.36 kJ

    (negative means heat is released)
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